Sulfur trioxide, an essential intermediate in the manufacturing of sulfuric acid, is produced industrially via the Contact Process. The balanced symbol equation for this equilibrium reaction is:
2SO2(g)+O2(g)⇌2SO3(g)2\text{SO}_2(\text{g}) + \text{O}_2(\text{g}) \rightleftharpoons 2\text{SO}_3(\text{g})2SO2(g)+O2(g)⇌2SO3(g)
The reaction is carried out in a closed system.
State how you can tell from the equation that this reaction is reversible.
What is meant by the term closed system?
When dynamic equilibrium is reached, which of these statements are correct?
Select two correct statements:
The equilibrium position can be altered by changing the reaction temperature. Suggest one other change that could be made to the reaction conditions to alter the equilibrium position.
A chemical plant predicts they will produce 1250 tonnes of sulfur trioxide. They actually produce 925 tonnes of sulfur trioxide. Calculate the percentage yield of sulfur trioxide.
State why this reaction has an atom economy of 100%. Use the balanced symbol equation.
Practise OCR GCSE Chemistry Equilibria with exam-style questions for Foundation and Higher tier. 35 questions, matched to the OCR GCSE Chemistry (J248) specification and written in Paper 1 and Paper 2 (Foundation Tier) or Paper 3 and Paper 4 (Higher Tier) style. Every question includes a full worked solution and mark scheme, so you can see where marks are awarded rather than just whether you got the answer right.